When heated with sulfuric or phosphoric acid, cyclohexanol, C6H11OH is converted to cyclohexene, C6H10. The balanced chemical equation for the reaction is shown below. C6H11OH(l) → C6H10 (l) + H2O(l) If the percent yield is 83%, what mass of cyclohexanol must we use to obtain 25 g of cyclohexene?

Answer 1

Billions of kilograms of urea, are produced annually for use as a fertilizer. The reaction used is given below.
NH3(g) + CO2(g) → CO(NH2)2(s) + H2O(l)
The typical starting reaction mixture has a 3:1 mole ratio of NH3 to CO2. If 47.7 g urea forms per mole of that reacts, what is the

2.2.1. Theoretical yield;
2.2.2. Actual yield;
2.2.3. Percent yield?

Answer 2

m=30g